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Reaction Kinetics - 6
1.
The two steps involved in the gas phase reaction
X+2Y XY2 are shown below
i. X+Y slow XY
vv. XY+Y fast XY2
What is the rate equation for the overall reaction?
a) Rate= K[x]0[y]2
b) Rate = K[xy]1[y]1
c) Rate= K[x]0[y]1
d) Rate = K [x30][y]1
2.
1. The distribution of molecular kinetic energies is with in a gas at temperatures T1 and T2 are shown in the diagram.
Which one of the following statements correctly explains why a small increase in temperature leads to a significant increase in the rate of a gaseous reaction?
a) The activation energy of the reaction is less when gases are at high temperature.
b) The frequency of collision between molecules with kinetic energy greater than the activation energy is greater at high temperature.
c) The frequency of collision between molecules is greater at a higher temperature.
d) The average kinetic energy of the molecules is slightly greater at a high temperature.
3.
The reaction of acidified, aqueous potassium iodide with aqueous hydrogen peroxide.
2I(aq)+H
2
O
2
(aq)+2H+(aq) I2(aq)+2H
2
O(l) is thought to involve the following steps:
H
2
O
2
+I- H
2
O+OI- (Slow)
OI-H+ HOI (Fast)
HOI- +H+ I2+H2O (Fast)
Which one of the following conclusion can not be drawn from this information?
a) Acid acts as a catalyst.
b) The iodide ion is oxidized by hydrogen peroxide
c) The reaction is first order with respect to iodide ion.
d) The rate determining step is H
2
O+I- H
2
O+OI-
4.
When a reaction occurs in many steps than the slowest step is.
a) Mechanism determining step.
b) Rate determining step
c) Enthalpy determining step
d) None of the above.
5.
The rate of reaction between two specific time intervals is called.
a) Average rate of a reaction.
b) Instantaneous rate of reaction.
c) Rate of a reaction.
d) None of the above.
6.
Decomposition of Ozone take place according to the following equation
To the following equation
2O
3
(g) 3O
2
(g)
Rate equation for the reaction is Rate k=[O
3
}2[O
2
]-1
What is the order of the reaction?
a) Zero
b) 1
c) 2
d) 3
7.
Half life period of a first order reaction is independent of
a) Presence of catalyst
b) Conditions of temperature
c) Initial concentration of the compound
d) All the above.
8.
Dilatometer method is useful for the reactions that involve.
a) Small volume changes in solutions.
b) Ionic species
c) Where reactant absorb U.V visible or infrared radiation.
d) Change in refractive indices.
9.
The energy of activation of forward reaction is less than that of backward reaction in.
a) Endothermic reactions
b) Exothermic reaction
c) Isothermic reaction
d) None of the above
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